Solid silver chromate is added to pure water at 25oC, and some of the solid rema

Question

Solid silver chromate is added to pure water at 25oC, and some of the solid remains undissolved. The mixture is stirred for several days to ensure that equilibrium is achieved between the undissolved Ag2CrO4 (s) and the solution. Analysis of the equilibrated solution shows that its silver ion concentration is 1.2 x 10-4 M. Assuming that silver chromate dissociates completely in water when it dissolves, and that there are no other equilibria involving Ag+ or CrO42- ions in the solution, calculate Ksp for this compound.

Explanation / Answer

Ag2CrO4(s) 2 Ag+(aq) + CrO42-(aq) Ksp = [Ag+]^2[CrO42-] Since [Ag+] = 1.2 X 10^-4, [CrO42-] = [Ag+] / 2 = 6 X 10^-5 M Plugging these into the equation for Ksp gives: Ksp = (1.2 X 10^-4)^2 (6.0 X 10^-5) = 8.6 X 10^-13

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